CH3 „Ph Ph. „CH3 H-SO4 > (А), HSO4 (B) 9. OH Product (A) & (B) respectively in the above reaction are : (а) Ph - С-NH -CHз, Ph - С-NH - СНз (Ъ) СНз - С-NH-Ph, СH3 - С-NH- Ph (c) Ph - С-NH - СН3, СНз — С-NH - Ph (d) CHз - С-NH-Ph, Ph - С-NH -СHз

CH3 „Ph Ph. „CH3 H-SO4 > (А), HSO4 (B) 9. OH Product (A) & (B) respectively in the above reaction are : (а) Ph - С-NH -CHз, Ph - С-NH - СНз (Ъ) СНз - С-NH-Ph, СH3 - С-NH- Ph (c) Ph - С-NH - СН3, СНз — С-NH - Ph (d) CHз - С-NH-Ph, Ph - С-NH -СHз

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 116IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...

See similar textbooks

Related questions

Q: alculate the percent ionization of formic acid (HCO2H) in a solution that is 0.152 M in formic acid.…

A: % ionization = [H+] /[ HA] intial X 100 As we know the initial concentration of formic acid is 0.152…

Q: Please show step by step... Thanku!

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: 5. At 25°C, calculate the molar H3O+ and OH-1 concentrations of the following: b. 0.0600 M NH3 c.…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Determine the H3O+ of a .230 M solution of formic acid. (Ka for formic acid 1.8•10^-4) Determine the…

A: Given that: initial concentration of formic acid = 0.230 M Ka for formic acid= 1.8×10-4 To find:…

Q: Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.222 M in formic acid…

A: The pH of the solution is calculated in accordance with the Henderson-Hasselbach- equation.

Q: What is the pH of a solution that is 0.400M in formic acid and 1.00M in sodium formate? (Ka formic…

Q: The molar H;O*concentration in 0.010M (ethylamine) C,H;NH2 (Ka for C,H;NH;*= 2.5× 105) is.... .....…

Q: 2.4 8 (a) Define in words the following: (1) Ka (ii) p.Ka I (b) Calculate the pH of 0.0005 mol dm³…

Q: 1. Acidity CI COOH COOH HO CI 1 2. Basicity NH2 NH2 NH2 NH2 CH3 CH3 H3C H3C 3. Stability 2. 4.

Q: The pH of a 0.057M solution of 3-hydroxypropanoic acid (HC,H,O,) is measured to be 2.88. Calculate…

Q: The value of Ka for phenol (a weak acid) , C,H5OH , is 1.00×10-10 . Write the equation for the…

A: Phenol acts as a weak base that means the hydrogen attached to -OH group in phenol is removed as a…

Q: An acid has a Ka = 7.77 x 10-4. Is it stronger or weaker than an acid with Ka = 7.77 x 10-3 ? A.…

A: We have to compare the acid strength.

Q: Which of the following is the strongest acids? A. Benzoic acid, K₂ = 6.25 x 10-5. B. Formic acid, K₂…

A: pKa value: pKa value negative logarithm of the acid dissociation constant (Ka). pKa = -logKa Low pKa…

Q: Calculate [OH-] of NaBrO, 0.810M; KaHBrO = 2.0 x 10-9. Group of answer choices 4.5 x 10-4 2.0 x 10-5…

Q: OUL UI 3 points. The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where…

Q: 6. Arrange the following 0.01 M substances in order of increasing pH. HNO3: pK, = -1.38 HNO2: pka =…

Q: Calculate the p-value for each of the indicated ions Na+, Cl- and OH- in a solution that is 0.0585…

A: Given, Na+, Cl- and OH- in a solution that is 0.0585 M in NaCl and 0.0846 M in NaOH H+, Cl- and…

Q: a. [CH3 COOH] = 0.85 M, [CH;CO0-] = 0.45 M (the pK, for acetic acid is 4.74) pH = b. [Н,РО, ] 3 0.50…

Q: Calculate the pH of a 0.355 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.

A: Given : concentration = 0.355 M Ka = 1.30 × 10-5

Q: 2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: Welcome to bartleby !

Q: Q2 : At 25°C, K = 3.40 x 10-3 S m-1 for 0.00100 M NH4OH. Values of Lo are: NH4C1 = 0.01497, NaOH…

Q: Hydroxide (-OH) can react as a Brønsted–Lowry base (and remove a proton), or a Lewis base (and…

A: Hydroxide (-OH) can react as a Brønsted–Lowry base (and remove a proton), or a Lewis base (and…

Q: What is the pH of a solution containing 0.30 M CH₃COONa and 0.10 M CH₃COOH? The Ka of CH₃COOH is 1.8…

Q: 3. The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Calculate the pH of a solution that is 0.112 M in sodium formate (NaHCO2) and 0.266 M in formic acid…

A: The given information is: Conc. of sodium formate (NaHCO2) = 0.112 M Conc. of formic acid (HCOOH) =…

Q: (b) 0.15 moldm of benzoic acid (CeHsCOOH; Ka of benzoic acid = 6.3 x 10-5 moldm- %3D 3)

A: Acid dissociation constant measures the acidic strength of an acid. Higher the value of Ka, higher…

Q: 1. Benzoic acid is a weak carboxylic acid that undergoes proton transfer with water. When a 0.125 M…

Q: HO он OH O The predominate form of benzene-1,2,3-tricarboxylic acid cannot be determined from the…

Q: For 1-3. Calculate the pH, pOH and [OH-] of black coffee which is 5×10^-5 MH+ 20. 1. What is the…

A: The given data contains, H3O+=5×10-5M

Q: Which one of the following correctly shows the equilibrium for the weak base quinoline, CsHN? A)…

Q: Acetic acid has a Ka = 1.8 x 10- 2 points 5 Determine the pH of a O.2 M acetic acid solution *…

Q: Pyridine is a weak base with K, = 1.7x10-10. %3D C3H5N(aq) + H20) C5H5NH" (aq) + OH Write the K…

Q: How do I solve for the reactant?

A: Acetic acid has carbon, hydrogen and oxygen in it and acetic acid in its standard state is a…

Q: LAH 1. NaH Ph- A 2. PHCH Br он OH A Ph. B Ph- Ph Ph он 2. A Ph OH B Ph. Ph Ph он Ph 3. A Ph. B Ph-…

Q: The pH of 0.25 M methylamine is 11.98 at 25 °C. The [OH-] at equilibrium is given below. What is the…

Q: Calculate the pH of a solution that is 0.374 M CH3COOH and 0.489 M CH3COONa. Ka of CH3COOH is 1.8 *…

A: Given :- Concentration of CH3COOH = 0.374 M Concentration of CH3COONa = 0.489 M Ka of CH3COOH =…

Q: To prepare a solution of chloroacetic acid (HACL) with pH = 2.87, the solution need only to have a…

Q: What is the pH of 0.15M solution of acetic acid? Ka of acetic acid (CH3COOH) is (Ka = 1.8x10-5 )

A: The PH of a solution is defined as : The negative…

Q: Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0…

A: When weak acid is titrated with strong base, the resultant solutionwill have unionized acid and salt…

Q: At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10$moldm3. c. Calculate the pH…

A: We will calculate both parts with the help of given information

Q: Which of the following relationships in INCORRECT? Assume T = 25°C. O pH + pOH = 14.00 %3D…

A: pH is the indicator of acidic nature of a solution. Any solution with pH equal to 7 is considered…

Q: S HAC HAC Listening is everythi... Courses 20 of 34 If [H+] = 2.33 x 10-3 M, what is the [OH-] of…

A: Given, [H+] = 2.33×10-3 M

Q: If you mix equal molar quantities of NH3 (Kb = 1.8 x 10-5) and CH3CO2H (Ka= 1.8 x 10-5), the…

A: Given that the solution contains equal molar concentrations of NH3 and CH3COOH. Also given Kb of NH3…

Q: Consider the following general equilibrium expression. aA(g) + bB(g)= CC(g) + dD(g) At 25 °C, if Kc…

A: We know that relationship between Kc and kp. Kp= KC(RT)∆ng ∆ng is the difference of gaseous moles of…

Q: Of the following which is a strong base? Select one: a. H2SO4 b. HCl c. NaOH d. NH3 e. NaCl Which…

A: A strong base is a species that can dissociate completely and give hydroxide ions or accepts protons…

Q: Brz -> la. Ph Br Br Br B. ph C. ph' Br A. Ph Br CHC13 (3. Ph h koH CI Cl Ci CI cl B. Ph D. C. A. Ph…

A: In this question we have to tell the product of the reaction.

Q: 2. 3. Ph-CO-Ph + N2H/HO" - » Ph-CH2 Ph Ans 4. Ph-CO-H + Ph-CO-H+ NAOH --> Ph-CO-OH + PHCH2-OH Ans 5.…

Q: What is the pH of 0.121M C6H5CH2COOH? C6H5CH2COOH + H2O ⇌ H3O+ + C6H5CH2COO- Ka = 4.9 x 10-5

Q: What is the pH of a solution that is 0.41 M in sodium acetate and 0.65 M in acetic acid? (for…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Calculate the pH of a solution that is 0.111 M in sodium formate (NaHCO2) and 0.253 M in formic acid…

A: The solution contains formic acid which is a weak monoprotic acid and salt of its conjugate base i.e…

Question

CH3
„Ph
Ph.
„CH3
H-SO4
> (А),
HSO4
(B)
9.
OH
Product (A) & (B) respectively in the above reaction are :
(а) Ph - С-NH -CHз, Ph - С-NH - СНз (Ъ) СНз - С-NH-Ph, СH3 - С-NH- Ph
(c) Ph - С-NH - СН3, СНз — С-NH - Ph (d) CHз - С-NH-Ph, Ph - С-NH -СHз

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
(c) Calculate the pH of 0.5 mol/L sodium hydrogen carbonate, NaHCO3. The Ka,1 of carbonic acid, H₂CO3, is 4.3 x 10-7. Нансез END
Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. CH:NH:CI(aq) + NaOH(aq) 4- 2+ | ]3+ 1 3 4 6 7 8 D4 15 Do ) (s) (1) (g) (aq) Na H C CI Reset • x H2O Delete 1L 2. +
Classify each of the following compounds as an acid, base, or both. Be sure to answer all parts. CH,CH,OH (select) Y CH,CH,CH,CH; |(select) v CH;CO.CH3 (select) Y
(a) Calculate the percent ionization of 0.00310 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b) Calculate the percent ionization of 0.00310 M butanoic acid in a solution containing 0.0790 M sodium butanoate. % ionization = %
(b) What is the pH of 0.39 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 10-4.)
3. Buffer solutions are used by the human body to maintain a constant pH for biochemical processes such as enzyme activity. In addition, buffer is used in baby shampoo and soap to maintain the pH, thereby preventing rashes on the baby. Given an ethanoic acid, CH-COОH with Kа %3 1.85 х 105. (а) Calculate the pH of a buffer solution containing 0.150 mol/L ethanoic acid and 0.150 mol/L sodium ethanoate using the Henderson-Hasselbalch equation. Give the proportion (ratio) for [CH;COO-] : [CH;COOH] with the same concentration that we should mix to produce a buffer solution of pH 5.00. (b)
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that hypochlorous acid is 3.0 x10-8 , which is a stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) calculate the Kb values for the CHCOO- and ClO- .
5. List the following compounds in order from strongest acid to weakest acid: CH4 CH;COOH CH;OH CHCI»OH 6. Which of the following are likely to act as Lewis acids and which as Lewis bases? Which might act both ways? (a) CH3CH2OH (d) (СH3)3B (b) (CHҙ)2NH (e) H3C+ (c) MgBr2 (f) (CH3)3P
Complete the balanced molecular reaction for the following weak base with a strong acid: Na CIO2(aq) + H2SO«(aq) – 4- |2+ 3+ 04+ 1 4 6. 7 8 9 Do (s) (1) (g) (aq) Na CI S H H2O OH Reset x H2O Delete 1L LO
The acid dissociation constants for sulfurous acid are: Ka1 3D 1.2 х 10-2 and Ka2 - 6.6 х 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.
If the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity constant, Kp, of CICH20-? You do not need to make a simplifying assumption CICH,0-(aq) + H2O(1) СICH-OОH(aq) + ОН (аq) K½ = ?